Posted by hannah on Tuesday, January 12, 2010 at 11:10pm.
The ions are titanium(III) and chromate. What you have, however, is not two ions; rather, a compound, titanium(III) chromate
Are you sure it is an ion? What is the ionic charge?
There are various forms of titanium chromate.
As Bob notes above it is necessary to indicate the oxidation state of the titanium as it can have +2, +3 and +4 oxidation state.
If the above is a neutral compound it would be titanium (III) chromate.
If, as you indcate, it is an ion then you are missing a charge on the ion. So possibilities might be:
[Ti2(CrO4)3]2-
which could be
bis(tetraoxochromato(VI))titanium (II)
[Ti2(CrO4)3]2+
bis(tetraoxochromato(VI))titanium (IV)
I am not sure of the stability of the various chromates, but I guess this is an academic naming exercise.
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